Draw the...?

Question

draw the lewis structure and indicate the direction of the bond dipole for these two single bonds: C-I and P-Se

Answer 1

in order to draw the lewis structure, add up the valence electrons (valence electrons is = to group # for each element) of each element in the molecule. Then divide that number by two which will represent each 'pair' of electron. Distribute the pair of electrons the best you can so that each will have 8 electrons around it. Only elements of C, N, O, or S can double bond to each other so there won't be any double bonding in this case.

memory isn't fresh on what dipole bond movement is....

But i think the movement goes in the direction of the more electronegative element. The most electronegative element is Chlorine on the periodic table. That means the trend of electronegativity increases across a period but decreases down a period. With this trend predict which direction the movement goes.

Answer 2

Let x be a C electron and *'s I electrons. Draw x* between C and I and two *'s around the other three sides of I. Put a "small +" over the C and a "small -" over the I to indicate the charges on these atoms.

The radii of P and Se are large, so they will not form P=Se bonds. Let x be a P electron and * an Se electron. Put x* between P and Se. Don't worry about other x's and *'s, because the problem does not give a compound, so you don't know what and where they are. The Pauling electronegativity of P is 2.1 and of Se 2.4. So put a "small +" charge over P and a "small -" charge over Se.